CHEMISTRY COMMUNITY

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Yes, you know that Kw is 1.0x10^-14 and you have OH- so you can find H3O+ by using Kw=[H3O+][OH-]

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Hypobromite ion is the conjugate base of hypobromous acid. From the table 12.1, the pKa of hypobromous acid is 8.69. We know that pKa+pKb=14. To get pKb, take 8.69 from 14 and you get 5.31. From table 12.2, we know that the pKb for C17H19O3N is 5.79.The pKb of hypobromite is smaller, which means tha...

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Yes, you can also think that as the pKa gets higher, the acid gets weaker and same for bases.

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Why do we use pKa instead of Ka?

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We know that HCl, HBr, and HI are strong acids but why is HF a weak acid?

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I make bad chemistry puns.... but only periodically

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Is there a difference in calculation when calculating atm or bar when finding K?

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How can you tell which structure has higher or lower energy? For example in 3.54, we have to identify which structure has the lowest energy.

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Structure B is better because it shows that S has a lower formal charge when the double bonds are created which makes it more stable.

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I know that when there is a dipole, there is a negative charge with the atom with more electronegativity and more of a positive charge on the opposite side. That's when it becomes a polar bond.

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I think you can determine if a bond is ionic if the electronegativity difference is greater than 2. If the electronegativity difference is less than 1.5, it's a covalent bond.

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When do we know when finding the formal charge is more important than using the octet rule?

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In 2.29 part c), I don't understand why the maximum number of electrons is 8 if n=2. Can someone please explain?

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In a) and in b), the configuration doesn't follow Hund's rule so it must be at an excited state. In c), the configuration doesn't follow Aufbau's principle which means that it would also be at an excited state. d) is the only configuration that follows Aufbau's principle and Hund's rule which means ...

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I think molecular weight and molar mass have different units because molecular weight comes from the total amount of the atomic mass in a molecule and molar mass is the amount of mass per mole of a molecule.

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Can someone please explain how after you calculate the amount of excess reactant, you would find the amount of limiting reactant needed to react with the excess reactant that is not used?

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I know from physics, that amplitude and energy are proportional. So the bigger the amplitude, the more energy. I'm not completely sure if it relates to the energy of a photon but that could get you thinking.

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The question asks: Lines of the Balmer series of the hydrogen spectrum are observed at 656.3, 486.1, 434.0, and 410.2 nm. What is the wavelength of the next line in the series?

I know that you can use Rydberg's formula to solve this but how could you solve this without using the Rydberg's formula?

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So how I thought of it was that the question is asking how much energy is in that 1.00 mol of sodium. After you multiply avogadro's constant with the energy from part A, you get 203x10^5 J/mol. But if you think about what the question is asking for, it says how much energy is per that mole. So reall...

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So after you get 2.2513x10^-14 J, that is your E in the formula. You can use the two formulas given: E=h(nu) and c=(lambda)(nu). Since nu is in both formulas, you can substitute them. when you substitute for nu, the new equation you get is E=hc/lambda. In order to find lambda, you can make the equat...

CHEMISTRY COMMUNITY

Search found 20 matches

Re: Homework problem 12.25

Re: 12.49

Re: Relationship between pKa and pKb

Re: pKa vs Ka

HCl vs. HF

Re: Post All Chemistry Jokes Here

calculating K

Energy in lewis structures

Re: Quick Question about SO4

Re: Polar vs. nonpolar

Re: Bonds

formal charge vs. octet

Re: Exercise 2.29

Re: Question 2.39

Re: Molar Mass

Excess reactant

Re: Amplitude of the wave [ENDORSED]

chapter 1 question 57

Re: Chapter 1 Number 19 [ENDORSED]

Re: Exercise 1.23 Pg 27 Ch 1